question archive Consider the equation: KClO3>>>>KCl + 3/2O2 Assign oxidation states to each element on each side of the equation

Consider the equation: KClO3>>>>KCl + 3/2O2 Assign oxidation states to each element on each side of the equation

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Consider the equation: KClO3>>>>KCl + 3/2O2 Assign oxidation states to each element on each side of the equation.

Reactants: ___K ___Cl ___O  and Products: ___K ___Cl ___O Which element is oxidized? Which is reduced?

 

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Answer:

KClO3 ---> KCl+ 3/2 O2

In KCLO3 the oxidation number of potassuim is +1, chlorine is +5, oxygen is -2

In KCl has oxidation number , potassium +1 and chlorine is -1

Oxygen molecule has oxidation number zero

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